Allotropes of Carbon: Diamond and Graphite

Introduction to Allotropes

• Definition: Allotropes are different structural forms of the same element in the same physical state.
• Examples of Carbon Allotropes: Diamond, Graphite, Fullerenes, Graphene.

Diamond

• Structure:
  • Giant covalent structure.
  • Each carbon atom forms four covalent bonds with other carbon atoms.
  • Creates a regular 3D pattern.
• Properties:
  • Very hard and strong due to strong bonds.
  • High melting point.
  • Electrical conductivity: Does not conduct electricity (no free electrons or ions).

Graphite

• Structure:
  • Giant covalent structure.
  • Each carbon atom is bonded to three other carbon atoms.
  • Atoms arranged in hexagons forming large flat sheets.
  • Layers held together by weak forces (not covalent bonds), allowing layers to slide over each other.
• Properties:
  • Relatively soft compared to diamond due to weak inter-layer forces.
  • High melting point (strong covalent bonds within layers).
  • Electrical conductivity: Conducts electricity and heat due to delocalised electrons (spare electron from each carbon atom).

Other Forms of Carbon

• Graphene:
  • A single layer of graphite.
  • Can be isolated and used to create other structures.
• Fullerenes:
  • Structures made from isolated graphene layers (e.g., spheres and tubes).

Conclusion

• Covered properties and structure of diamond and graphite.
• Next video will explore graphene and fullerenes.
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